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Midterm Review Study Guide
Unit 1: Measurement and Calculations
Non-zero digits: are _________ significant
Non zero digits include:
Ex. 5891
How many sig figs?
Zero Digits:
Captive zeros: are _________ significant
Ex. 22.05
How many sig figs?
Captive are surrounded by _______________
Ex. 100203.601 has 9 sig figs
Leading zeros: are _________ significant
Ex. 0.25 has 2 sig figs
Ex. 0.0036 How many sig figs?
Trailing zeros: are only significant ____________is present
Ex. 500
How many sig figs?
Ex. 500.
How many sig figs?
_____ m/L/g = _____Kilo (k)
_____ m/L/g = Hecto (h)
_____ m/L/g = Deka (dk)
1 Base = 1base
Deci (d) = _____ m/L/g
Centi (c) = _____ m/L/g
Milli (m = _____ m/L/g
Sig Figs and Operations
Sig Figs are counted when ___________________________________
Sig Figs are NOT counted when ___________________________
Multiplying, Dividing or powers: round to the ________ number of significant figures
Ex: 4.56 x 1.4 How many sig figs should answer contain?
Adding or Subtracting: round to the least number of digits _______ the decimal
Ex: 4.56 + 1.2 How many sig figs should answer contain?
How to round numbers:
1. Determine how many sig figs you need.
2. Draw a line after that number
3. If the number after the line is between 0-4, the number before the line stays the same
If the number is 5 or higher, the number before the line should round up
Examples:
(Round to 2 sig figs) 1.33
1.4 3 3 is between 0-4, so the number before the line stays the same 1.4
Scientific Notation
How is Scientific Notation Written?
Convert to Decimal Form: 2.8 X 103
Convert to Scientific Notation: 0.744
Unit 2 Science of Matter
All matter has 3 major characteristics
1. It has _____________
2. It takes up _____________
3. It is made of particle called ___________
All matter exists in three states:
1. __________(fixed shape, fixed volume)
2. __________ (variable shape, fixed volume)
3. __________ (variable shape, variable volume)
Density: is the amount of _________ present in a given _____ of substance. It is expressed as g/mL or g/cm3
The formula for density is
D=
Example:
A student finds that 23.50 mL of soda weighs 35.06 g. What is the density?
Specific Heat: is
The unit for specific heat is
The formula for specific heat is
Q=
Example: Calculate the joules of energy required to heat 454 g of water from 5.4 degrees
Celsius to 98.6 degrees Celsius
Chemical Properties vs. Physical Properties
List examples of Chemical properties
List examples of Physical Properties
Physical Changes vs. Chemical Changes
List examples of Physical Changes
List examples of Chemical Changes
Unit 3: Elements
Vocabulary
Proton:
Neutron:
Electron:
Cation:
Anion:
Nucleus:
Isotope:
Diatomic:
What are the diatomics?
Atomic #
Mass #
CompoundCompounds ALWAYS contain:
Chemical Formula:
Chemical formulas include:
Rules for writing Formulas:
1.
2.
3.
8
O
Oxygen
16.00
Examples:
Write the complete chemical symbol for the ion with 31 protons, 39 neutrons, and 28 electrons
Ionic Compounds:
Must have a net charge of _____
Alkali Metals:
Alkali Earth Metals
Transition Metals
Metalloids
Halogens
Noble Gases
Actinide
Label the Periodic Table Accordingly
Unit 4: Modern Atomic Theory
Wavelength
Frequency
Proton
Excited State
Ground State
Orbital
Pauli Exclusion Principle
Core Electrons
Ionization Energy
What is the trend on the Periodic Table?
Atomic Radius
What is the trend on the Periodic Table?
Electron Configuration
Orbit
Electrongs
Understand how to label Orbital Diagrams:
Ex: Magnesium (Mg)
# of Electrons
Order in which orbitals fill
1s, 2s…..
How to determine Valence Electrons
When wavelength goes up, frequency goes ________
When wavelength goes down, frequency goes ________
Unit 5:
Ion (def):
Elements want to bond? Why? Who do they want to look like? Why?
Covalent Bond (def):
Example:
Ionic Bond (def):
Example:
Type I:
Located?
Writing the name:
What comes first?
What comes second? How is it written
What are the charges on the periodic table (by column)
Type II:
Located:
Writing the Name
What comes first?
What comes second? How is it written?
Type III:
Examples:
Polyatomics
Common polyatomics and charges
Acids start with what element? _____________________
There are two types of Acids
1. Ones that _______ oxygen
2. Ones that _____ ________ oxygen
Steps to name acids that have oxygen:
Steps to name acids that don’t have oxygen:
Roman Numerals:
1=I
2 = II
3=
4=
5=
6=
Prefixes:
1=
2=
3=
4 = tetra
6=
8=
9=
Unit 6 Study Guide
Definitions:
Single replacement
Example:
Double replacement
Example:
Decomposition
Example:
Combustion:
Example:
Synthesis
Example:
Subscript:
What does it tell us?
Coefficient:
When is it used?
Precipitate
Product
Where is it located when writing an equation?
Reactant
Where is it found when writing an equation?
Abbreviations
Solid =
Liquid =
Gas (also referred to as vapor)=
Aqueous =
Important information
Diatomic:
What are the 7 diatomics?
**Understand how to write and balance a chemical equation. Practice problems:
#1. If calcium carbonate is heated strongly, carbon dioxide gas is driven off, leaving a residue of of calcium
oxide. Write the balanced chemical equation for this process:
#2. Balance: H2O2
#3. Balance: K2CO3
H2O + O2
2O
+ CO2
#4. When Copper (II) oxide is boiled in an aqueous solution of sulfuric acid, it produces Copper (II) sulfate and
water. Write the balanced chemical equation for this process: